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Published byJulianna Lowndes Modified over 2 years ago

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o “K” : Manipulation of K Kp verse Kc

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Write an equilibrium constant expression for any chemical reaction. The concentrations of solids and solvents (e.g., water) are not included in equilibrium constant expressions Recognize that a large value of K (K>> 1) means the reaction is product-favored. A small value of K (K << 1) indicates a reactant-favored reaction. Use equilibrium constants to calculate the concentration of a reactant or product at equilibrium. Apply Le Chatelier’s principle to predict the effect of a disturbance on a chemical equilibrium: a change in temperature, a change in concentrations, or a change in volume or pressure for a reaction involving gases

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Calculate an equilibrium constant given the reactant and product concentrations at equilibrium Apply the idea of the reaction quotient (Q) to decide if a reaction is at equilibrium. Q = K; reaction is at equilibrium Q

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K is designated as K c when Equilibrium concentrations are expressed in terms of reactant and product concentration, M (moles per liter). K is designated as K p, when concentrations of gases are represented by partial pressures (amount of gas measured in atm or Kpa)

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Know how K changes as different stoichiometric coefficients are used in a balanced equation and when equation is reversed Know that, when two chemical equations are added to give a net equation, the value of K for the net equation is the product of the values of K for the summed equations

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Kp

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2NO 2 + O 2 ↔ 2NO 3 + C +4 2H 2 O + C H 4 CO 2 +4 H 2 H 2 + I 2 ↔ 2HI

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S(s) + O 2 (g) ---> SO 2 (g) Fe 3+ (aq) + SCN - (aq) FeSCN 2+ 3+ N 2N 3 H 2 (g) + N 2 (g) 2N H 3 (g)

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Kp verse Kc

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K 3 = K 1 * K 2 K 3 = K 1 K 2 K w = K a * K b

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